Calcium Hydroxide -Lime-

There are many chemicals available on the market today that are suitable for use as neutralization chemicals.
The most commonly used chemicals are discussed in an article available here:
Neutralization Chemicals.

Calcium Hydroxide Ca(OH)2

Calcium Hydroxide [Ca(OH)2].
Also commonly referred to as slaked lime or hydrated lime; calcium
hydroxide is formed as a result of hydrating lime (calcium oxide,
CaO). Lime is by far the most economically favorable alkaline
reagent to use for acid neutralization. Lime is significantly
cheaper than caustic (NaOH), but is much more difficult to handle.

As with
magnesium hydroxide, Lime is not very soluble in water.
Although the reaction times of lime are substantially less than
magnesium hydroxide, lime is difficult to handle because it is
handled as a slurry.

Ca(OH)2 is divalent, yielding two
moles of (OH)2 for every one mole of Ca(OH)2.
When compared to
caustic
(NaOH), which is monovalent, twice the neutralizing power is
available for a given molar volume of lime, thus contributing to
the economy of lime. As with magnesium hydroxide, lime is normally
delivered in dry crystalline form. This must then be mixed with
water to form a slurry to be delivered to the process. The ease
with which caustic (sodium hydroxide) can be handled makes it far
more favorable than lime, at least for low volume applications.

Lime is a slurry that will rapidly separate
from solution. The storage tank must be constantly agitated and
chemical delivery lines must be kept in motion. Typically
recirculation loops are employed with a metering valve, inline, for
chemical delivery. Static lines are not acceptable because the
slurry will separate, and lines will plug, over time.

Lime offers very significant advantages when
the precipitation of metals or fluorides is the goal. Calcium salts
are normally quite insoluble, and due to the fact that lime is
divalent, sludge densities are normally much higher than those
formed with caustic (NaOH).

Lime is an excellent choice for acid neutralization. If volumes are
relatively low, and precipitation of metal or fluoride ions is not
paramount, then caustic (NaOH) may be the better choice because it
is easier to handle.